Net Ionic Equations
A net ionic equation shows only the species that actually participate in a chemical reaction, omitting spectator ions that remain unchanged.
Key Concepts
- Spectator ions: Ions present in solution that do not take part in the reaction
- Molecular equation: Shows all reactants and products as compounds
- Ionic equation: Shows all strong electrolytes dissociated into ions
- Net ionic equation: Eliminates spectator ions to focus on the chemical change
Steps to Write Net Ionic Equations
- Write the balanced molecular equation.
- Dissociate all strong electrolytes into ions.
- Identify and cancel spectator ions.
- Write the resulting net ionic equation.
Example
-
Molecular equation:
NaCl(aq) + AgNO₃(aq) → AgCl(s) + NaNO₃(aq) -
Ionic equation:
Na⁺(aq) + Cl⁻(aq) + Ag⁺(aq) + NO₃⁻(aq) → AgCl(s) + Na⁺(aq) + NO₃⁻(aq) -
Net ionic equation:
Ag⁺(aq) + Cl⁻(aq) → AgCl(s)
Importance
- Focuses on the actual chemical change
- Simplifies analysis of precipitation, acid-base, and redox reactions
- Useful in stoichiometry calculations and predicting reaction outcomes
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